Problem: How much heat is required to warm 1.50 L of water from 26.0 oC to 100.0 oC? (Assume a density of 1.0 g/mL for the water.)

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We’re being asked to determine the amount of heat (Q) needed to raise the temperature of 1.50 L water from 26 ˚C to 100 ˚C


The amount of heat Q is given by:


Q=mcT


where m = mass (in grams), c = specific heat, ΔT = change in temperature = final T – initial T.


We’re given the volume of water hence, we need to convert it to its mass by multiplying with the density.


Recall:

density=massvolume


 We’re given the following values:

volume = 1.50 L

density = 1.00 g/mL

c = 4.186 J/g • ˚C (found in books and on the internet)

ΔT = 100 ˚C – 26 ˚C = 74 ˚C

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Problem Details

How much heat is required to warm 1.50 L of water from 26.0 oC to 100.0 oC? (Assume a density of 1.0 g/mL for the water.)

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What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Calorimetry concept. You can view video lessons to learn Calorimetry. Or if you need more Calorimetry practice, you can also practice Calorimetry practice problems.